Question

Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H2] initial rate of reaction 0.948 M 2.32 M 0.116 M/s 0.948 M 0.662 M 0.0331 M's 4.24 M 2.32 M 2.32 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate * k=0

Answer 1

Rate law of the reaction can be written as - R = k [Ne7 [H₂ g (1) Where k = rate Constant n = order of reac with respect to CN2] y = Order of reac with respect to [hz] from given data's ; RR = 0.116 M = K (0.948) (2.3278 -(2) Rp = 0.0331 ^ = K (0.9489" (0.66278 -(3) R3 2 2.32 4 = K (4:24)" (2:32)8 -14) - (30594 = 3.5 1431 2 butting 4.4725)^=_207 PL=2 the value of n and y in (2)

R = 0.116 = K (0.948)?(232) M3 = 0.116 M-28-1 0.899 72.32 R = 0.0556 m-25-1 Rate law from equation (1) R = 0.0556 [N2]° [Hz]' Auss